Summary

Summary Lewis Formulas

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Course
Ch 101 (CH101)

Institution
Boston University

Lewis formulas, or Lewis structures, are diagrams that represent the bonding between atoms in a molecule and show lone pairs of electrons. They help illustrate how atoms share or transfer electrons to achieve a stable electron configuration, usually following the octet rule. These structures are es...

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chaptf.TT#FOMas ¥ÉµÑ F. bond length → 141pm
an atom , and, that can Fz Clzbond length -7199 pm
electron lntheoutershell associated
with
Valence electrons -
an
ofachemicalbondlf-heoutershelllsno-closedilnaslng.IE covalent
Brz bond length → 228pm
-

participate in the formation

µ
'm order -10 forma shared P " "
one valence electron
bond , both atomsinthebond contribute, 1
,
bond length → 26> pm

:& ! :& ÷

a.me#aaiEEii .ua&oii. -@aa?:%*i:q•B d%•a% iµ
:
.ci! : → :&! :&
.
' '
-
.
-1
:
a .
F-
Distribution of Valence electrons
if
:& :-& :&
r•→n*i•1
:

:÷ :
tf Molecular
Molecular
model of
:& - -
&: .
Br , ☐ fz
Model of

between atoms These electron pairs are known as
Coty
covalent bonds -

sharing of electron pairs
-

of attractive and repulsive forces between

µY
shared pairs or
bonding pairs , and the stable balance
atoms
double bond -
a chemical bondmwhlchtwo Pairs of electrons are shared between

two atoms

Lewis formula diagrams that show the bonding between atoms
-
Ofa molecule , aswell as

* ÷ ÷ ÷" " " " "" triple bond a chemical bond in which three pairs of electrons are shared between
-
÷.

'¥÷É÷!¥¥¥÷*¥;÷ÉÉ÷•÷¥;÷É•0E÷.÷¥É:¥¥•÷ .
µfff←
two atoms
12
lone electron pairs pair of resonance form another
way of drawing alewisdot structure fora given
-
-
valence electrons

tnatarenotsnareawitnanotneratomina covalent
bond ¥ compound

molecular

relatively
crystal
weak intermolecular
-
substances that have

binding Cdryice )
@@qgq⑨¥ Bond : average bond length / pm Average bond energy / AJ
C- 0 142 0.581
bond length -
distance between the centers of
I -21
two C = 0 121
covalently bonded atoms ; determined by the
number of bonded electrons ( bond order )
O 581
153
'

c - c
Octect rule
to attain
nearest that of
an outer

a
-
atoms gain
shell electron
noble gas
or lose electrons
configuration *. C=C 134
I. 02

1<35
f, CIC 120
guppy , .

° -266
N -
N 145
free radical -
an atom or molecule
containing one or more unpaired electrons
inyalencyshellorouterorb,+
and capable of independent
is existence
N=N 118 0.698

electronegativity
-
periodic property; used to predict the polarity of chemical bonds NIN 113 1.58

Vector -

quantity that has botha
magnitude and a direction ; used to specify the

a*•ñ9&
position , velocity > and momentum of .
a
particle , or -10 Specify a force .

I
'
'
W i'
Ii : Silicon tetrachloride HF bond length -792 pm c " c
l Lewis structure Hi Y
H
yf¥
H
HF 5
HCl bond /
length → 128pm -
:&! -

Yi
-
&! :
µBr bond length → 141pm
I
C
,, → 11
120°F
:
?! : HI bond length → 16hpm
, c c
cJ°\H
⑧µÑ⑧
'
1-1 /
atoms are almost always terminal / ✗ c/ µ
\
Hydrogen µ
atoms in Lewis Formulas I 1
H H

It Is not octect rule
always possible to
satisfy the
using only single
bonds
HC/
2C 41-1 12
H
02+14 NONE =

f f (2×4)+(4×1)
- -

not possible to satisfy
H H
the octect rule for each

⑥µ
carbon atom with onlythe NH -2 N 21-1 + I
8
µ remaining valence
=
two

µ electrons ; short two (1×5)+(2×1)
" / electrons
\
' .

c=c
H'
'
1-1 A NHI N 41-1 -
l = 8
Violates the (1×5)+(2×4)
µ -1¥ HBR
.

octetruie

t
electrons
:N=_ N : a species with one or more unpaired
~ called a free radical

KADESH
Is
formula
Lewis electron dot
Resonance hybrid Isa superposition of Lewis Formulas .

µ . any .gg .

I →
ii.
→ -0 11¥
¥:-O
'
cannot satisfy octectrule
:O
'

⑦
.

-0
HI
i.i-Q.or.H-i.ci

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